Question

How does the normality of an oxalic acid solution relate to its molarity?

Answer 1

Hint: Oxalic acid is an organic acid having the formula $ HOOC-COOH $ and the IUPAC name ethanedioic acid. It is the most basic of the dicarboxylic acids. It's a white crystalline solid that dissolves in water to create a colourless solution. It gets its name from the fact that oxalic acid was first extracted from flowering plants of the genus Oxalis, sometimes known as wood-sorrels. Although oxalic acid is found naturally in many foods, it can be harmful if consumed in large amounts or when skin contact is sustained.

Complete answer:
In chemistry, normality is one of the terms used to describe the concentration of a solution. It is sometimes referred to as the equivalent concentration of a solution and is abbreviated as ‘N.' It is mostly used to determine the amount of reactive species in a solution, as well as during titration reactions and circumstances requiring acid-base chemistry.
Molar concentration is a measurement of a chemical species' concentration in a solution, specifically a solute's concentration, in terms of the amount of substance per unit volume of solution. The number of moles per litre, abbreviated as mol/L in SI units, is the most widely used unit for molarity in chemistry. A solution with a concentration of 1 mol/L is known as a molar solution, or 1 M.
It is given the formula $ \text{N = Molarity }\!\!~\!\!\text{ }\!\!\times\!\!\text{ Basicity }\!\!~\!\!\text{ = Molarity }\!\!\times\!\!\text{ Acidity} $
A diacid is oxalic acid. To attain neutrality, each equivalent of acid takes two equivalents of base. Of course, $ p{{K}_{a}}2 $ will be significantly higher than $ p{{K}_{a}}1 $ .
  $ \mathrm{HOOC}-\mathrm{COOH} .2 \mathrm{H}_{2} \mathrm{O} $
The molar mass is $ =2\cdot 12+6\cdot 16+6\cdot 1=126g\text{ }mo{{l}^{-1}} $
The acid's basicity is two since its molecule generates $ 2 H^{+} $ ions in its aqueous solution.
Hence the equivalent mass of the acid is known to be $ =\dfrac{\text { molar mass }}{\text { basicity }}=\dfrac{126}{2}=63 \dfrac{g}{\text { equivalent }} $
A solution's normalcy $ =\dfrac{\text { No. of gm-equivalent }}{L}=\dfrac{\text { strength in } \mathrm{g} / \mathrm{L}}{\text { equivalent mass }} $
  $ =\dfrac{\text { strength in } \mathrm{g} / \mathrm{L}}{63 \dfrac{g}{\text { equivalent }}} $
So upon knowing the strength in $ \dfrac{g}{L} $ and dividing it by $ 63 \dfrac{g}{\text { equivalent }} $ we may simply obtain the oxalic acid solution's normality.

Note:
Gathering information regarding the equivalent weight of the reactive substance or the solute is the first tip that students may use. To understand about the molecular weight and valence, consult a textbook or reference book.
The number of g equivalents of the solute is calculated in the second phase.
It is important for students to remember that the volume is measured in litres.
Finally, using the formula and substituting the values, normalcy is determined.